Question

The standard Gibbs energy change at `300K` for the reaction `2AhArrB+C` is 2494. `2J`. At a given time, the composition of the reaction mixture is `[A]=1/2, [B]=2` and `[C]=1/2`. The reaction proceeds in the
`(R=8.314JK//"mol"e=2.718)`

Answer 1

the equilibrium reaction is :
`2A hArr B+C`
`DeltaG^(Theta) =- 2.303 RT " log " K_(c)`
`DeltaG^(Theta) = 2494.2 J " mol" ^(-1) , R =8.314 JK^(-1) " mol "^(-1) , T=300 K.`
`log K_(c) =- (2494.2 J " mol "^(-1))/((2,303) xx(8.314 JK^(-1) mol^(-1))(300K))=- 0.434`
`K_(c) Antilog (- 0.434) =0.367`
`[A]= 1/2, [B] = 2 and [C] = 1/2.`
`" For the reaction : " " " Q_(c) ([B][C])/([A]^(2)) = (2xx1//2)/(1//2xx1//2)=4`
Since `Q_(c)gt K_(c)` , reaction is expected to proceed in the backward direction .